Q1. (a) State what is meant by the term activation energy of a reaction. (c) State in general terms how a catalyst increases the rate of a chemical reaction. The curve below shows the Maxwell Boltzmann distribution of molecular energies, at a constant temperature, in a gas at the start of a reaction. On this diagram the most probable molecular energy at this temperature is indicated by the symbol E mp and the activation energy by the symbol E a. Consider the following changes. (iii) The number of molecules is increased at constant temperature. The temperature is decreased without changing the number of molecules. A catalyst is introduced without changing the temperature or the number of molecules. For each of these changes state how, if at all, the following would vary: the value of the most probable energy, E mp the number of molecules with the most probable energy, E mp the area under the molecular energy distribution curve the number of molecules with energy greater than the activation energy, E a (1) (Total 15 marks) Page 1 of 5
Q. Hydrogen is produced by the reaction between steam and methane when the following dynamic equilibrium is established. CH 4 (g) + H O(g) CO(g) + 3H (g) ΔH = +06 kj mol 1 (a) Use Le Chatelier s principle to predict the separate effects of an increase in temperature and of an increase in pressure on the yield of hydrogen obtained in the above reaction. In each case, explain your answer. (6) State how, and explain why, the use of a catalyst might or might not change the equilibrium yield of hydrogen, and also the amount of hydrogen produced, in a given time. (4) (Total 10 marks) Q3. (a) Below is a Maxwell Boltzmann curve showing the distribution of molecular energies for a sample of gas at a temperature T. Label the axes on the diagram above. What does the area under the curve represent? (iii) State why this curve starts at the origin. (4) State what is meant by the term activation energy. Page of 5
The rate of a chemical reaction may be increased by an increase in reactant concentration, by an increase in temperature and by the addition of a catalyst. State which, if any, of these changes involves a different activation energy. Explain your answer. Change(s)... Explanation... (5) (Total 9 marks) Q4. (a) Define the term activation energy for a reaction....... Give the meaning of the term catalyst....... (c) Explain in general terms how a catalyst works....... Page 3 of 5
(d) In an experiment, two moles of gas W reacted completely with solid Y to form one mole of gas Z as shown in the equation below. W(g) + Y(s) Z(g) The graph below shows how the concentration of Z varied with time at constant temperature. (iii) On the axes above, sketch a curve to show how the concentration of W would change with time in the same experiment. Label this curve W. On the axes above, sketch a curve to show how the concentration of Z would change with time if the reaction were to be repeated under the same conditions but in the presence of a catalyst. Label this curve Z. In terms of the behaviour of particles, explain why the rate of this reaction decreases with time. (6) (Total 1 marks) Page 4 of 5
Q5. (a) A sample of a gas was sealed into a flask at temperature T and pressure P. The Maxwell Boltzmann distribution of energies for the molecules in this sample is shown below. Using the axes above, sketch the curve that you would expect if this sample of gas at pressure P had been cooled. Label this curve X. Using the axes above, sketch the curve that you would expect if another sample of the same gas was sealed in the same flask at the original temperature, T, but at a higher pressure. Label this curve Y. (4) Gas A decomposes slowly to form gases B and C. An equilibrium is established as shown by the following equation. A(g) B(g) + C(g) ΔH is positive In terms of the behaviour of molecules, state what must happen before molecules of A can react to form B and C. Explain why the decomposition of A is faster at higher temperatures. (4) Page 5 of 5
(c) The graphs below show how, starting from A alone, the concentration of A varies with time at temperatures of 300 K and 30 K for the reversible reaction given in part. Suggest why, as shown on the graphs, the concentration of A remains constant after a time. Explain why, at 30 K, the concentration of A falls to a lower value compared with the reaction at 300 K. (3) (Total 11 marks) Q6. The diagram below represents a Maxwell Boltzmann distribution curve for the particles in a sample of a gas at a given temperature. The questions below refer to this sample of particles. (a) Label the axes on the diagram. On the diagram draw a curve to show the distribution for this sample at a lower temperature. Page 6 of 5
(c) In order for two particles to react they must collide. Explain why most collisions do not result in a reaction.... (d) State one way in which the collision frequency between particles in a gas can be increased without changing the temperature.... (e) Suggest why a small increase in temperature can lead to a large increase in the reaction rate between colliding particles.......... (f) Explain in general terms how a catalyst works.......... (Total 10 marks) Q7. Gas G decomposes as shown in the equation below. G(g) X(g) + Y(g) (a) Draw, on the axes below, a Maxwell Boltzmann distribution curve for a sample of G in which only a small proportion of molecules has energy greater than the activation energy, E a. (3) Page 7 of 5
Define the term activation energy....... (c) At any time, most of the molecules of G have energy less than the activation energy. Suggest why, at a constant temperature, most of G eventually decomposes....... (d) State the effect, if any, of adding a catalyst on the time required for G to decompose, compared with a similar sample without a catalyst. Explain in general terms how the catalyst has this effect. Time for decomposition... Explanation...... (3) (Total 10 marks) Q8. The curve below shows how the volume of oxygen evolved varies with time when 50 cm 3 of a.0 mol dm 3 solution of hydrogen peroxide, H O, decomposes at 98 K. (a) State how you could use the curve to find the rate of reaction at point A.... Page 8 of 5
Sketch curves, on the above axes, to illustrate how the volume of oxygen evolved would change with time if the experiment was repeated at 98 K using the following. 100 cm 3 of a 1.0 mol dm 3 solution of H O. Label this curve X. 5 cm 3 of a.0 mol dm 3 solution of H O in the presence of a catalyst. Label this curve Y. (4) (c) Hydrogen peroxide decomposes more rapidly in the presence of aqueous hydrogen bromide. The decomposition proceeds as shown by the following equations. H O + HBr HBrO + H O HBrO + H O H O + O + HBr Write an equation for the overall reaction. Define the term catalyst. (iii) Give two reasons, other than an increase in the reaction rate, why these equations suggest that hydrogen bromide is behaving as a catalyst. Reason 1... Reason... (5) (Total 10 marks) Q9. (a) Define the term activation energy for a chemical reaction. Draw, with labelled axes, a curve to represent the Maxwell Boltzmann distribution of molecular energies in a gas. Label this curve T 1. On the same axes, draw a second curve to represent the same sample of gas at a lower temperature. Label this curve T. Use these curves to explain why a small decrease in temperature can lead to a large decrease in the rate of a reaction. (8) Page 9 of 5
(c) Give one reason why most collisions between gas-phase reactants do not lead to a reaction. State and explain two ways of speeding up a gas-phase reaction other than by changing the temperature. (5) (Total 15 marks) Q10. The gas-phase reaction between hydrogen and chlorine is very slow at room temperature. H (g) + Cl (g) HCl(g) (a) Define the term activation energy....... Give one reason why the reaction between hydrogen and chlorine is very slow at room temperature....... (c) Explain why an increase in pressure, at constant temperature, increases the rate of reaction between hydrogen and chlorine....... (d) Explain why a small increase in temperature can lead to a large increase in the rate of reaction between hydrogen and chlorine....... (e) Give the meaning of the term catalyst....... Page 10 of 5
(f) Suggest one reason why a solid catalyst for a gas-phase reaction is often in the form of a powder.... (Total 9 marks) Q11. The diagram below shows the Maxwell Boltzmann distribution of molecular energies in a sample of a gas. (a) State which one of X, Y or Z best represents the mean energy of the molecules. Explain the process that causes some molecules in this sample to have very low energies. On the diagram above, sketch a curve to show the distribution of molecular energies in the same sample of gas at a higher temperature. (3) (c) Explain why, even in a fast reaction, a very small percentage of collisions leads to a reaction. Page 11 of 5
Other than by changing the temperature, state how the proportion of successful collisions between molecules can be increased. Explain why this method causes an increase in the proportion of successful collisions. Method for increasing the proportion of successful collisions... Explanation... (4) (Total 9 marks) Q1. The diagram below shows the Maxwell Boltzmann energy distribution curve for a sample of gas at a fixed temperature. E a is the activation energy for the decomposition of this gas. (a) On this diagram sketch the distribution curve for the same sample of gas at a higher temperature. (3) What is the effect of an increase in temperature on the rate of a chemical reaction? Explain your answer with reference to the Maxwell Boltzmann distribution. Effect... Explanation... Page 1 of 5
What is the effect of the addition of a catalyst on the rate of a chemical reaction? Explain your answer with reference to the Maxwell Boltzmann distribution. Effect... Explanation... (6) (Total 9 marks) Q13. Carbon monoxide and hydrogen are used in the manufacture of methanol. An equilibrium is established according to the following equation. Cu catalyst CO(g) + H (g) CH 3 OH(g) H = 9l kj mol 1 (a) Give two features of a reaction at equilibrium. Feature 1...... Feature...... Explain why an increase in temperature causes a decrease in the equilibrium yield of methanol.......... (c) State what is meant by the term catalyst. State the effect, if any, of the copper catalyst on the position of this equilibrium at a fixed temperature. Page 13 of 5
(d) Two methods are used to produce carbon monoxide from natural gas. Equations for these two methods are shown below. Method 1 CH 4 + H O CO + 3H Method CH 4 + CO CO + H The manufacture of methanol from these sources of carbon monoxide has been described as carbon neutral............. Show how combining the equations from these two methods can lead to the 1: mol ratio of carbon monoxide to hydrogen required for this synthesis of methanol. (Total 8 marks) Q14. A group of students devised an experiment which they believed would enable them to investigate the strength of the intermolecular forces between ethyl ethanoate molecules (CH 3 COOCH CH 3 ) and trichloromethane molecules (CHCl 3 ). They mixed exactly 0.10 mol of each of the two liquids in a copper calorimeter and recorded the following results. The starting temperature of both liquids was the same. Mass of 0.10 mol of ethyl ethanoate / g 8.80 Mass of 0.10 mol of trichloromethane / g 11.95 Increase in temperature ( T) on mixing / K 9.5 (a) Write an expression for the heat change (q) which relates mass (m), specific heat capacity (c) and change in temperature ( T). Page 14 of 5
Calculate the amount of heat required to increase the temperature of 8.80 g of ethyl ethanoate by 9.5 K during the mixing process. (You should assume that c for ethyl ethanoate = 1.9 J g 1 K 1 ) (iii) Calculate the amount of heat required to increase the temperature of 11.95 g of trichloromethane by 9.5 K during the mixing process. (You should assume that c for trichloromethane = 0.96 J g 1 K 1 ). (iv) Using the values from parts (a) and (a) (iii), calculate the molar enthalpy change in kj mol 1 for the mixing process. The students deduced that the heat change was due only to the formation of intermolecular forces between ethyl ethanoate molecules and trichloromethane molecules. Ignoring all experimental errors, give one reason why the students may have made an incorrect deduction....... (Total 6 marks) Page 15 of 5
Q15. Barium can be extracted from barium oxide (BaO) in a process using aluminium. A mixture of powdered barium oxide and powdered aluminium is heated strongly. The equation for this extraction process is shown below. 3BaO(s) + Al(s) 3Ba(s) + Al O 3 (s) Some standard enthalpies of formation are given in the table below. Substance BaO(s) Al O 3 (s) ο H f / kj mol 1 558 1669 (a) State what is meant by the term standard enthalpy of formation. (3) State why the standard enthalpy of formation of barium and that of aluminium are both zero. (iii) Use the data to calculate the standard enthalpy change for the reaction shown by the equation above. (3) Suggest the major reason why this method of extracting barium is expensive. Using barium oxide and aluminium powders increases the surface area of the reactants. Suggest one reason why this increases the rate of reaction. Page 16 of 5
(c) Write an equation for the reaction of barium with water. A solution containing barium ions can be used to test for the presence of sulfate ions in an aqueous solution of sodium sulfate. Write the simplest ionic equation for the reaction which occurs and state what is observed. Simplest ionic equation Observation... (iii) State how barium sulfate can be used in medicine. Explain why this use is possible, given that solutions containing barium ions are poisonous. Use... Explanation... (Total 14 marks) Q16. Sodium thiosulfate solution (Na S O 3 ) reacts slowly with dilute hydrochloric acid to form a precipitate. The rate of this reaction can be studied by measuring the time (t) that it takes for a small fixed amount of precipitate to form under different conditions. The fixed amount of precipitate is taken as the amount needed to obscure a cross on paper. The equation for this reaction is shown below. Na S O 3 + HCl NaCl + S + SO + H O (a) Identify the insoluble product of this reaction which forms the precipitate.... When this reaction takes place, the collision between the reacting particles requires an activation energy. State what is meant by the term activation energy....... Page 17 of 5
(c) In terms of particles, explain why, at a fixed temperature, you might expect the rate of this reaction to double when the concentration of sodium thiosulfate is doubled and the concentration of hydrochloric acid remains the same............. (d) State what is meant by the term rate of reaction. Consider the description of the way in which this experiment is carried out. Use your understanding of the term rate of reaction to explain why it is possible to use a simplified formula as a measure of the rate of this reaction. (Total 7 marks) Q17. Nitric acid is manufactured from ammonia in a process that involves several stages. (a) In the first stage, ammonia is converted into nitrogen monoxide and the following equilibrium is established. 4NH 3 (g) + 5O (g) 4NO(g) + 6H O(g) H = 905 kj mol 1 The catalyst for this equilibrium reaction is a platinum rhodium alloy in the form of a gauze. This catalyst gauze is heated initially but then remains hot during the reaction. In terms of redox, state what happens to the ammonia in the forward reaction. Suggest a reason why the catalyst must be hot. (iii) Suggest a reason why the catalyst remains hot during the reaction. Page 18 of 5
(iv) State how a catalyst increases the rate of a reaction. In the second stage, nitrogen monoxide is converted into nitrogen dioxide. The equation for the equilibrium that is established is shown below. NO(g) + O (g) NO (g) H = 113 kj mol 1 Explain why the equilibrium mixture is cooled during this stage of the process............. (c) In the final stage, nitrogen dioxide reacts with water as shown by the following equation. NO (g) + H O(l) H + (aq) + NO 3 (aq) + HNO (aq) Give the oxidation state of nitrogen in each of the following. NO.. NO 3... HNO (3) (Total 10 marks) Page 19 of 5
Q18. An equation for the equilibrium reaction between hydrogen, iodine and hydrogen iodide is shown below. H (g) + I (g) HI(g) (a) The curve in the diagram below illustrates the reaction profile for this equilibrium reaction without a catalyst. (iii) (iv) Draw on the diagram a curve to illustrate the reaction profile for this equilibrium reaction with a catalyst. Use the diagram to deduce whether the formation of hydrogen iodide from hydrogen and iodine is exothermic or endothermic. State what the diagram suggests about the sum of the bond enthalpies for the reactant molecules compared with the product molecules. In terms of p and q, identify the following for this equilibrium without a catalyst. A value for the activation energy for the forward reaction... A value for the overall enthalpy change for the forward reaction A mixture of H (g) and I (g) was allowed to reach equilibrium. State the effect of a catalyst on the rate of attainment of this equilibrium. Page 0 of 5
State and explain the effect of an increase in total pressure on the rate of attainment of this equilibrium. Effect of an increase in pressure on rate... Explanation... (3) (Total 10 marks) Q19. The diagram below shows a Maxwell Boltzmann distribution for a sample of gas at a fixed temperature. E a is the activation energy for the decomposition of this gas. (a) On this diagram, sketch the distribution for the same sample of gas at a higher temperature. With reference to the Maxwell Boltzmann distribution, explain why an increase in temperature increases the rate of a chemical reaction. Page 1 of 5
Dinitrogen oxide (N O) is used as a rocket fuel. The data in the table below show how the activation energy for the decomposition of dinitrogen oxide differs with different catalysts. N O(g) N (g) + O (g) Ea / kj mol 1 Without a catalyst 45 With a gold catalyst 11 With an iron catalyst 116 With a platinum catalyst 136 Use the data in the table to deduce which is the most effective catalyst for this decomposition. Explain how a catalyst increases the rate of a reaction. (Total 7 marks) Q0. The rate of a chemical reaction is influenced by the size of the activation energy. Catalysts are used to increase the rates of chemical reactions but are not used up in the reactions. (a) Give the meaning of the term activation energy............. Page of 5
Explain how a catalyst increases the rate of a reaction............. (c) The diagram below shows the Maxwell Boltzmann distribution of molecular energies, at a constant temperature, in a gas at the start of a reaction. On this diagram the most probable molecular energy at this temperature is shown by the symbol E mp The activation energy is shown by the symbol E a To answer the questions 1 (c) to 1 (c) (iv), you should use the words increases, decreases or stays the same. You may use each of these answers once, more than once or not at all. State how, if at all, the value of the most probable energy (E mp ) changes as the total number of molecules is increased at constant temperature. State how, if at all, the number of molecules with the most probable energy (E mp ) changes as the temperature is decreased without changing the total number of molecules. (iii) State how, if at all, the number of molecules with energy greater than the activation energy (E a ) changes as the temperature is increased without c hanging the total number of molecules. Page 3 of 5
(iv) State how, if at all, the area under the molecular energy distribution curve changes as a catalyst is introduced without changing the temperature or the total number of molecules. (d) For each of the following reactions, identify a catalyst and name the organic product of the reaction. The fermentation of an aqueous solution of glucose. Catalyst... Name of organic product... The hydration of but--ene. Catalyst... Name of organic product... (Total 1 marks) Page 4 of 5
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